ANSWER KEY
Station One:
Types of Compounds
Type I: Ionic Compound
-
Has a metal NOT from the transition metal section of the PT and a
nonmetal/polyatomic ion.
Does NOT use Roman numerals in the name
Type II: Ionic Compound
-
Has a metal from the transition metal section of the PT and a nonmetal/polyatomic
ion.
Uses Roman numerals in the name
Type III: Covalent Compound
-
Made of 2 nonmetals.
Uses prefixes in the name
Type Acids:
-
H is ALWAYS the first element in the compound
The name always says acid in it!
If there is NO oxygen in the formula, it’s a binary acid and you HAVE to use the
prefix hydro- in the name.
If there is oxygen in the formula, it’s an oxyacid and it will end in either –ic acid
(comes from –ate) or –ous acid (comes from –ite).
Directions: Identify the type of compound for each substance.
1. N2O3
Type III
2. H2CO3
Type Acid (oxyacid)
3. Aluminum sulfate
Type I
4. Cobalt (III) nitride
Type II
5. HBr
Type Acid (binary acid)
6. Tetraphosphorous decoxide Type III
7. K3PO4
Type I
8. MnF2
Type II
9. Strontium chloride
Type I
10. Au2(SO3)3
Type II
Station 2: Writing Formulas
Type I: Ionic Compounds
-
Write the symbol and charge of the metal, use the periodic table to determine the
charge.
-
Write the symbol and charge of the nonmetal/polyatomic ion.
-
Criss-cross the charges.
o If you cross a number to a polyatomic ion, put the ion in parentheses first.
Type II: Ionic Compounds
-
Write the symbol and charge of the metal, the Roman Numerals tell you the charge
for the metal
-
Write the symbol and charge of the nonmetal/polyatomic ion.
-
Criss-cross the charges.
o If you cross a number to a polyatomic ion, put the ion in parentheses first.
Type III: Covalent Compounds
-
Write the symbol for the first element; change the prefix to a subscript.
-
Do the same thing for the 2nd element.
Directions: Write the symbol for the following compounds.
1. Magnesium bromide
MgBr2
2. Iron (III) sulfide
Fe2S3
3. Diphosphorous pentoxide
P2O5
4. Potassium nitrite
KNO3
5. Copper (II) hydroxide
Cu(OH)2
6. Sulfur trioxide
SO3
7. Barium phosphate
Ba3(PO4)2
8. Vanadium (V) chlorite
V(ClO2)5
9. Xenon hexafluoride
XeF6
Station 3: Naming compounds
Type I: Ionic Compounds
-
Write the name of the metal
-
Write the name of the nonmetal, change the ending to –ide.
OR
-
Write the name of the polyatomic ion.
Type II: Ionic Compounds
-
Write the name of the metal.
-
You need to write the original charge of the metal as a Roman Numeral. You will
have to un-criss-cross the charges to do so.
-
Write the name of the nonmetal, change the ending to –ide.
OR
-
Write the name of the polyatomic ion.
Type III: Covalent Compounds
-
Write the name of the first element.
-
Change the subscript to a prefix.
-
Do the same for the 2nd element, just remember that the 2nd element must end in –ide.
Directions: Write the names of the following compounds.
1. Na2O
sodium oxide
2. CrI3
chromium (III) iodide
3. H2O
dihydrogen monoxide
4. CaCO3
calcium carbonate
5. Pd2(SO3)3
palladium (III) sulfate
6. IF7
iodine heptafluoride
7. Al(NO3)3
aluminum nitrate
8. AgNO2
silver (I) nitrite
9. CCl4
carbon tetrachloride
Station 4: Acids
Formulas
-
Is hydro- part of the name? Then there is NO oxygen in the formula!
o Write H+.
o Write the 2nd element’s symbol and charge.
o Criss-cross the charges.
-
If there is NO hydro, does it end in –ic acid or –ous acid?
o If it ends in –ic acid…

Write H+.

Write the symbol and charge of the polyatomic ion that ends in –ate.

Criss-cross charges.
o If it ends in –ous acid…

Write H+.

Write the symbol and charge of the polyatomic ion that ends in –ite.

Criss-cross charges.
Names
-
If there is NO oxygen in the formula, it’s a binary acid.
o Write the prefix hydroo Write the first part of the 2nd element
o End with –ic acid.
-
If there is oxygen in the formula, check out the polyatomic ion.
o Does the name of the polyatomic ion end in –ate?

Change –ate to –ic acid.
o Does the name of the polyatomic ion end in –ite?

Change –ite to –ous acid.
Directions: Write the formula for these acids.
1. Hydrofluoric acid
HF
2. Nitric acid
HNO3
3. Hydrosulfuric acid
H2 S
4. Nitrous acid
HNO2
Directions: Write the name for these acids.
5. H3PO4
phosphoric acid
6. H3N
hydronitric acid
7. HI
hydroiodic acid
8. H2SO3
sulfurous acid
Station 5: Balancing Chemical Equations
Use coefficients to make sure that you have the same number of atoms of each element on
the left and right side of the equation! Remember, a coefficient multiples through an entire
formula!
Directions: Balance the equations.
1. 2H2O(l) + Ba(s) → H2(g) + Ba(OH)2(aq)
2. 3Na2SO4(aq) + 2FePO4(aq) → 2Na3PO4(aq) + Fe2(SO4)3(s)
3. 2H2O2(aq) → 2H2O(l) + O2(g)
4. 2HBr(aq) + Ca(OH)2(aq) → CaBr2(aq) + 2H2O(l)
5. C5H12(l) + 8O2(g) → 5CO2(g) + 6H2O(g)
Station 6: Types of Reaction
-
Synthesis
o Reactant 1 + Reactant 2 → Product
o Ex. H2 + Cl2 → 2HCl
-
Desomposition
o Reactant → Product 1 + Product 2
o Ex. 2 NaCl → 2Na + Cl2
-
Single-replacement
o Element 1 + Compound 1 → Element 2 + Compound 2
o 2Li + MgSO4 → Mg + Li2SO4
-
Double-replacement
o 2 compounds switch ions
o NaNO3 + KBr → NaBr + KNO3
-
Combustion
o Hydrocarbon + Oxygen → Carbon dioxide + Water
o CH4 + 2O2 → CO2 + 2H2O
Directions: Identify the type of reaction for each equation.
1. H2O(l) + Ba(s) → H2(g) + Ba(OH)2(aq)
single-replacement
2. Na2SO4(aq) + FePO4(aq) → Na3PO4(aq) + Fe2(SO4)3(s)
double-replacement
3. H2O2(aq) → H2O(l) + O2(g)
decomposition
4. HBr(aq) + Ca(OH)2(aq) → CaBr2(aq) + H2O(l)
double-replacement
5. C5H12(l) + O2(g) → CO2(g) + H2O(g)
combustion
6. CaCO3(s) → CaO(s) + CO2(g)
decomposition
7. C2H5OH(l) + O2(g) → CO2(g) + H2O(g)
combustion
8. Na(s) + Al(OH)3(aq) → Al(s) + NaOH(aq)
single-replacement
9. Mg(s) + N2(g) → Mg3N2(s)
synthesis
10. Pb(NO3)3 + H2SO4(aq) → PbSO4(s) + HNO3(aq)
double-replacement